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bruno102

  • one year ago

Using the table provided, determine which of the following statements is true about the reaction of solid sodium with chlorine gas (2 Na (s) + 1 Cl2 (g) arrow 2 NaCl(s)) at 25 degrees Celsius and 1 atmosphere. The reaction produces no change in ΔG. The reaction is nonspontaneous. The reaction is spontaneous. The reaction produces a +ΔG.

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  1. bruno102
    • one year ago
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  2. bruno102
    • one year ago
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    I don't understand this one.

  3. Photon336
    • one year ago
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    I'll help you in a bit

  4. bruno102
    • one year ago
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    Ok thank you

  5. Photon336
    • one year ago
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    Ok so looking at your table, Notice two things. In the equation you have Na and cl2 So notice you have deltaG of formation which, the concept is the same for Hear of formation in the sense that naturally occurring elements have Delta g of formation of 0 So Na and chlorine gas have delta g of formation of 0

  6. Photon336
    • one year ago
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    You notice that the delta G of formation for NaCl is both large and negative. So it's spontaneous. Note delta g of formation is for one mole of the substance so in our case we would multiply this value by 2

  7. bruno102
    • one year ago
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    Okay

  8. bruno102
    • one year ago
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    So it is C?

  9. Photon336
    • one year ago
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    This kind of makes sense, for multiple reasons. Why it's so large. Technically chlorine wants that electron so badly and sodium wants to lose the electron to Achieve octet so, once the bond forms you'll release a lot of energy. You'll get a bond that's more like an ionic bond one in which electrons are transfered from Sodium to Cl, in NaCl

  10. Photon336
    • one year ago
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    Yes

  11. bruno102
    • one year ago
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    Thanks again. I have a couple I am going to post, just to check my answer.

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